What does it mean when components do not want to stay in the liquid phase?
It indicates a positive deviation from Raoult's Law.
What does it mean when components want to stay in the liquid phase?
It indicates a negative deviation from Raoult's Law.
p.12
Vapor Pressure and Boiling Point
What happens to the boiling point of a more volatile solvent?
It has a lower boiling point.
p.12
Vapor Pressure and Boiling Point
What is the effect of a less volatile solvent on vapor pressure?
It results in lower vapor pressure.
p.22
Colligative Properties
What is osmotic pressure?
The pressure required to stop the flow of solvent into a solution through a semipermeable membrane.
What happens to a gaseous solute under increased pressure?
It reaches a new equilibrium.
p.28
Boiling Point Elevation
What is the formula for boiling point elevation?
ΔT = Kb * m_solute, where m_solute is molality.
p.30
Colligative Properties
What do colligative properties depend on?
The number of solute particles, not their identity.
p.12
Vapor Pressure and Boiling Point
What is the relationship between volatility and vapor pressure?
More volatile solvents have higher vapor pressure.
What does Henry's Law describe?
The behavior of a gaseous component as a solute in a solution.
What is the initial stage in the process of increasing pressure on a gaseous solute?
The gaseous solute is at its original state before pressure is applied.
p.17
Vapor-Liquid Equilibria
What is the vapor-liquid equilibrium for pure toluene?
It describes the balance between the vapor and liquid phases of pure toluene.
p.9
Vapor Pressure and Boiling Point
What is the relationship between temperature and vapor pressure?
Higher temperature results in higher vapor pressure.
What indicates a negative deviation from Raoult's Law?
Less molecules in the gas phase than the ideal case.
p.15
Vapor Pressure and Boiling Point
What is a characteristic of an ideal solution regarding solvent vapor pressure?
It has a lower solvent vapor pressure.
What does Raoult's Law relate to?
The gaseous component resulting from the vaporization of a solvent.
What does the phrase 'like dissolves like' refer to?
It refers to the principle that polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes.
p.16
Vapor Pressure and Boiling Point
What is the effect of a salt solution on vapor pressure?
It has lower vapor pressure, leading to net condensation.
p.9
Vapor Pressure and Boiling Point
What is assumed when solvent is placed in a vacuum?
Gas components almost do not interact with each other.
p.6
Temperature Effects on Solubility
How does temperature affect the solubility of a gas in a solvent?
The solubility of a gas typically decreases with increasing temperature.
p.21
Colligative Properties
What does a negative trend indicate?
A decrease or decline in a particular variable.
p.21
Colligative Properties
What is the significance of identifying trends?
It helps in making predictions and informed decisions based on data.
p.23
Colligative Properties
What is osmotic pressure?
A colligative property that depends on the number of solute particles in a solution.
What does χ_solv stand for?
The mole fraction of the solvent.
What is P_solv° in the context of Raoult's Law?
The vapor pressure of the pure solvent.
p.12
Vapor Pressure and Boiling Point
What is the effect of a less volatile solvent on its boiling point?
It has a higher boiling point.
p.15
Vapor Pressure and Boiling Point
What effect do non-volatile solutes have on an ideal solution?
They lead to a lower solvent vapor pressure.
p.9
Vapor Pressure and Boiling Point
What happens in a region above a liquid when it is 'too empty'?
Net vapourization occurs.
What does Raoult's Law describe?
The relationship between the vapor pressure of a solution and the mole fraction of its solvent.
What indicates a positive deviation from Raoult's Law?
More molecules in the gas phase than the ideal case.
p.30
Colligative Properties
What is another example of a colligative property?
Freezing-point depression.
p.9
Vapor Pressure and Boiling Point
What concept is related to gas components not interacting in a vacuum?
Ideal gas and partial pressure.
p.25
Boiling Point Elevation
What does Kb stand for in the boiling point elevation equation?
Molal boiling-point elevation constant.
In Raoult's Law, what does the mole fraction represent?
The ratio of the number of moles of the solvent to the total number of moles of all components in the solution.
p.10
Boiling Point Elevation
What happens at the boiling point?
Vapor pressure equals atmospheric pressure.
p.8
Vapor-Liquid Equilibria
What is the role of a gaseous component in a container?
It can act as a solute or result from the vaporization of the solvent.
p.28
Molality and Molarity
What does molality depend on?
Moles of solute per kilogram of solvent.
p.25
Boiling Point Elevation
What effect does a nonvolatile solute have on the boiling point of a solvent?
It elevates the boiling point.
p.30
Colligative Properties
What is osmotic pressure?
A colligative property that depends on the number of solute particles.
p.26
Boiling Point Elevation
What does 'm_solute' represent in the boiling-point elevation equation?
The molality of the solute.
What does Henry's Law state about the concentration of dissolved gas?
C = kP, where C is the concentration of dissolved gas, k is Henry's law constant, and P is the partial pressure of the gas solute above the solution.
What occurs after increasing the pressure on a gaseous solute?
The system adjusts to a new equilibrium.
p.23
Colligative Properties
What is another example of a colligative property?
Freezing-point depression.
p.26
Boiling Point Elevation
What does Kb represent in the context of boiling-point elevation?
The molal boiling-point elevation constant.
p.28
Boiling Point Elevation
What is the relationship between boiling point elevation and molality?
Boiling point elevation is directly dependent on molality.
p.24
Molality and Molarity
What is the formula for molality (m)?
m = moles of solute / kilograms of solvent.
p.13
Vapor Pressure and Boiling Point
What is often assumed about solid solutes in terms of volatility?
They are assumed to be perfectly non-volatile.
p.23
Colligative Properties
What do colligative properties depend on?
The number of solute particles, not their identity.
p.27
Colligative Properties
What type of solid is glucose in solution?
A molecular solid present as individual molecules.
p.22
Colligative Properties
What are colligative properties?
Properties that depend on the number of solute particles in a solution, not their identity.
p.16
Vapor Pressure and Boiling Point
What happens during net condensation in a salt solution?
The vapor pressure decreases.
p.24
Molality and Molarity
How does molality differ from molarity?
Molarity uses solution volume, while molality uses solvent mass.
p.22
Colligative Properties
What is the effect of solute concentration on vapor pressure?
Adding solute decreases the vapor pressure of the solvent.
p.10
Boiling Point Elevation
What is the definition of boiling point?
The temperature at which vapor pressure equals atmospheric pressure.
p.7
Temperature Effects on Solubility
What is the general trend of solid solute solubility in water with temperature?
The solubility of most solids in water increases with temperature.
p.21
Colligative Properties
How can trends be summarized?
By analyzing the overall direction and magnitude of changes in data.
What happens to the amount of gas dissolved in a solution when the partial pressure of the gas above the solution increases?
The solubility of the gas increases.
p.17
Vapor-Liquid Equilibria
What happens to vapor-liquid equilibria when equal amounts of pure toluene and benzene are mixed?
The equilibrium will reflect the combined properties of both solvents.
p.17
Vapor-Liquid Equilibria
What is the vapor-liquid equilibrium for pure benzene?
It describes the balance between the vapor and liquid phases of pure benzene.
What does P_soln represent in Raoult's Law?
The observed vapor pressure of the solution.
p.22
Colligative Properties
How do colligative properties affect freezing point?
They lower the freezing point of a solution compared to the pure solvent.
p.29
Boiling Point Elevation
How do you calculate molality (m) of the solute?
m = moles of solute / kg of solvent.
What does Raoult's Law state?
The vapor pressure of a solvent in a solution is directly proportional to the mole fraction of the solvent.
What type of solutions does Raoult's Law apply to?
Ideal solutions, where the interactions between different molecules are similar to those between like molecules.
p.21
Colligative Properties
What does a positive trend indicate?
An increase or improvement in a particular variable.
p.28
Molality and Molarity
How is the number of moles of solute calculated?
Moles of solute = mass of solute / molar mass of solute.
p.16
Vapor Pressure and Boiling Point
What is the vapor pressure of pure water compared to a salt solution?
Pure water has higher vapor pressure, leading to net vaporization.
p.13
Vapor Pressure and Boiling Point
What is a characteristic of a non-volatile component?
It does not contribute to vapor pressure.
p.13
Vapor Pressure and Boiling Point
What happens to vapor pressure when less solvent molecules are present?
Vapor pressure decreases.
What is the formula for Raoult's Law?
P_solution = X_solvent * P°_solvent, where P_solution is the vapor pressure of the solution, X_solvent is the mole fraction of the solvent, and P°_solvent is the vapor pressure of the pure solvent.
What type of solutions does Modified Raoult's Law apply to?
Liquid-liquid solutions where both components are volatile.
p.7
Temperature Effects on Solubility
Are there exceptions to the trend of solid solute solubility with temperature?
Yes, the solubilities of some substances decrease with increasing temperature.
p.7
Temperature Effects on Solubility
What will be discussed in Chapter 12 regarding solubility?
The complexities of solid solute solubility trends with temperature.
p.26
Boiling Point Elevation
What does the symbol ΔT represent in the boiling-point elevation formula?
The change in boiling point.
p.24
Colligative Properties
Why is molality useful?
It describes properties that depend on atom counts, such as colligative properties.
p.16
Vapor Pressure and Boiling Point
What happens during net vaporization in pure water?
The vapor pressure increases.
p.12
Vapor Pressure and Boiling Point
How does the number of solvent molecules in the gas phase relate to volatility?
More volatile solvents have more solvent molecules in the gas phase.
p.13
Vapor Pressure and Boiling Point
What is the implication of mixing volatile and non-volatile components?
Non-volatile components lead to fewer solvent molecules in the gas phase.
How does the presence of a solute affect the vapor pressure of a solvent according to Raoult's Law?
The presence of a solute lowers the vapor pressure of the solvent.
p.1
Properties of Solutions
What course does Chapter 10 belong to?
CHEM 1011 General Chemistry A.
What phase will we focus on regarding enthalpy change?
Liquid solution (solvent & solution phase is liquid).
p.1
Properties of Solutions
What are the key concepts covered in the chapter?
Reactions, Thermodynamics, and Reaction Kinetics.
